If Delta H is the change in enthalpy,Delta U | vedclass

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(D) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ for a chemical reaction is given by the equation: $\

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$\Delta H > \Delta U$ when $N_P > N_r$

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(D) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ for a chemical reaction is given by the equation: $\Delta H = \Delta U + \Delta n_g RT$,where $\Delta n_g = N_P - N_r$ (change in the number of moles of gaseous species).If $N_P > N_r$,then $\Delta n_g > 0$,which implies $\Delta H > \Delta U$.If $N_P Therefore,the correct statement is $\Delta H > \Delta U$ when $N_P > N_r$.

If $\Delta H$ is the change in enthalpy,$\Delta U$ is the change in internal energy,$N_P$ is the number of moles of products,and $N_r$ is the number of moles of reactants,then which of the following is correct for a gaseous reaction?

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